Bonding: Shapes of molecules

Linear

                     Linear 

  • 2 electron pairs = 2 bonding pairs/0 lone pairs
  • Bond angle = 180 degrees
  • E.g. BeCl2           

                                          Image result for linear molecule (http://oer2go.org/mods/en-boundless/figures.boundless-cdn.com/32429/full/bpvhippzt8iblv68hvou.jpg)

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Trigonal planar

Trigonal planar

  • 3 electron pairs = 3 bonding pairs/0 lone pairs
  • Bond angle = 120 degrees
  • E.g. BF3

Image result for trigonal planar molecule

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Tetrahedral

Tetrahedral

  • 4 electron pairs = 4 bonding pairs/0 lone pairs
  • Bond angle = 109.5 degrees
  • E.g. CH4

                                                Related image

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Trigonal pyramidal

Trigonal pyramidal

  • 4 electron pairs = 3 bonding pairs/1 lone pair
  • Bond angle = 107 degrees
  • E.g. NH3

                                                   Image result for trigonal pyramidal molecule (http://upload.wikimedia.org/wikipedia/commons/thumb/d/d4/Ammonia-with-lone-pairs-3D-balls.png/240px-Ammonia-with-lone-pairs-3D-balls.png)

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Bent (v-shape)

Bent (v-shape)

  • 4 electron pairs = 2 bonding pairs/2 lone pairs
  • Bond angle = 104.5 degrees
  • E.g. H20

                                      Image result for bent molecule

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Trigonal bipyramidal

Trigonal bipyramidal

  • 5 electron pairs = 5 bonding pairs/0 lone pairs
  • Bond angle = 90/120 degrees
  • E.g. PF5

                                                      Image result for trigonal bipyramidal molecule

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Trigonal pyramidal/see-saw

Trigonal pyramidal/see-saw

  • 5 electron pairs = 4 bonding pairs/ 1 lone pair
  • Bond angle = 119/89 degrees
  • E.g. SF4

                                              Related image

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Trigonal planar/ T shape

Trigonal planar/ T-shape

  • 5 electron pairs = 3 bonding pairs/2 lone pairs
  • Bond angle = 89 degrees
  • E.g. ICl3

                                                               Image result for t shape molecule

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Octahedral

Octahedral

  • 6 electron pairs = 6 bonding pairs/0 lone pairs
  • Bond angle = 90 degrees
  • E.g. SF6

                                                                    Image result for octahedral molecule

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Square Planar

Square planar

  • 6 electron pairs = 4 bonding pairs/2 lone pairs
  • Bond angle = 90 degrees
  • E.g. XeF4

 Image result for square planar molecule

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Square pyramid

Square pyramid

  • 6 electron pairs = 5 bonding pairs/1 lone pair
  • Bond angle = 89 degrees
  • E.g. IF5

                                                Image result for square pyramid molecule (http://wps.prenhall.com/wps/media/objects/3311/3391094/imag0902/AAAVJJX0.JPG)

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